Interpretation:
The molar concentration of
Concept introduction:
Redox:
The reduction and oxidation reactions are occur simultaneously with in a single reaction is known as
Redox titration:
Redox titration is type of titration method to determine the amount of analyte that present in the given sample by redox reaction.
Mole:
Mole of the compound present in the solution is calculated by molarity concentration of the compound multiplied with litre volume of solution.
Mass:
Mass of the compound is calculated by mole of the compound is multiplied with molar mass of the compound.
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General Chemistry: Atoms First
- Write the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.arrow_forwardTriiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?arrow_forwardA 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ion, which was then precipitated with an excess of potassium chromate to give 2.012 g of barium chromate, BaCrO4. What is the formula of the compound?arrow_forward
- Calcium in blood or urine can be determined by precipitation as calcium oxalate, CaC2O4. The precipitate is dissolved in strong acid and titrated with potassium permanganate. The equation for reaction is 2MnO4(aq)+6H+(aq)+5H2C2O4(aq)2Mn2+(aq)+10CO2(g)+8H2O A 24-hour urine sample is collected from an adult patient, reduced to a small volume, and titrated with 26.2 mL of 0.0946 M KMnO4. How many grams of calcium oxalate are in the sample? Normal range for Ca2+ output for an adult is 100 to 300 mg per 24 hour. Is the sample within the normal range?arrow_forwardA soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?arrow_forward1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does the reaction of Ba(OH)2(aq) + H+PO4(aq) fit? acid-base and oxidation-reduction oxidation-reduction acid-base and precipitation precipitationarrow_forward
- Arsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent insect damage. Arsenic acid has three acidic protons. Say you take a 25.00-mL sample of arsenic acid and prepare it for titration with NaOH by adding 25.00 mL of water. The complete neutralization of this solution requires the addition of 53.07 mL of 0.6441 M NaOH solution. Write the balanced chemical reaction for the titration, and calculate the molarity of the arsenic acid sample.arrow_forwardThe active ingredients of an antacid tablet contained only magnesium hydroxide and aluminum hydroxide. Complete neutralization of a sample of the active ingredients required 48.5 mL of 0.187 M hydrochloric acid. The chloride salts from this neutralization were obtained by evaporation of the filtrate from the titration; they weighed 0. 4200 g. What was the percentage by mass of magnesium hydroxide in the active ingredients of the antacid tablet?arrow_forwardElemental bromine is the source of bromine compounds. The element is produced from certain brine solutions that occur naturally. These brines are essentially solutions of calcium bromide that, when treated with chlorine gas, yield bromine in a displacement reaction. What are the molecular equation and net ionic equation for the reaction? A solution containing 40.0 g of calcium bromide requires 14.2 g of chlorine to react completely with it, and 22.2 g of calcium chloride is produced in addition to whatever bromine is obtained. How many grams of calcium bromide are required to produce 10.0 pounds of bromine?arrow_forward
- Glycerol (C3H8O3) is commonly used as an additive to moisturizers. The amount of glycerol added can be determined by titration with permanganate in basic solution. 14MnO4(aq)+C3H8O3(aq)+20OH(aq)14MnO42(aq)+3CO32(aq)+14H2O How many milliliters of 6.15 M KMnO4 are required to completely react with 7.25 mL of an aqueous solution of glycerol (d=1.144g/mL) that is 51.6% by mass?arrow_forwardAn aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.arrow_forwardSodium chloride is used in intravenous solutions for medical applications. The NaCl concentration in such solutions must be accurately known and can be assessed by reacting the solution with an experimentally determined volume of AgNO3 solution of known concentration. The net ionic equation is Ag+(aq)+Cl(aq)AgCl(s) Suppose that a chemical technician uses 19.3 mL of 0.200-M AgNO3 to convert all the NaCl in a 25.0-mL sample of an intravenous solution to AgCl. Calculate the molarity of NaCl in the solution.arrow_forward
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